Given the following $\Delta$ H values, calculate the $\Delta$ H for the complete combustion of stearic acid.
$\begin{array}{ll}
\Delta \mathrm{H}(\mathrm{Kcal} / \mathrm{mol} .) & \text { Compound } \
-211.4 & \mathrm{C}_{17} \mathrm{H}_{35} \mathrm{COOH} \
0 & \text { Oxygen } \
-94 & \text { Carbon dioxide } \
-68.4 & \text { Water }
\end{array}$
A) -49 Kcal
B) -2096.2 Kcal
C) -2711.8 Kcal
D) 0 Kcal
E) 3071.8 Kcal

Question

Quizplus · Accepted Answer

The complete combustion of stearic acid ($\mathrm{C}_{17} \mathrm{H}_{35} \mathrm{COOH}$) can be represented by the equation:  $\mathrm{C}_{17} \mathrm{H}_{35} \mathrm{COOH} + 26\mathrm{O}_2 \rightarrow 18\mathrm{CO}_2 + 18\mathrm{H}_2\mathrm{O}$.  Using the given enthalpies:  $\Delta H = [18(-94) + 18(-68.4)] - [-211.4]$.  $\Delta H = [-1692 - 1231.2] + 211.4 = -2711.8 \text{ Kcal/mol}$.

Given the Following Δ\DeltaΔ H Values, Calculate The Δ\DeltaΔ H for the Complete Combustion of Stearic Acid

Given the Following $\Delta$ H Values, Calculate The $\Delta$ H for the Complete Combustion of Stearic Acid